Answer :
Answer:
4
Explanation:
Given reaction is
2A + 3B -> 2C
From the above reaction for every 2 moles of A, 2 moles of C is formed and therefore for every mole of A reacted, 1 mole of C is formed
Now in this case we have 4 moles of A and excess amount of B
So in this case the limiting reagent is A and the excess reagent is B
As in this case A is the limiting reagent so for 4 moles of A reacted, 4 moles of C is formed
But formation of 4 moles of C is just expected because it is just the maximum amount of C formed as during the reaction there can be losses as well if the reaction is not done properly
The reaction stoichiometric coefficient determines the moles of product and reactant in the reaction. 4 moles of A produces 4 moles of C.
What is the stoichiometric law?
The moles formed in the reaction are given by the stoichiometric coefficient through the stoichiometric law.
The stoichiometric law for the reaction states that, for the formation of 2 moles of C, 2 moles of A are required.
Thus, the moles of C formed by 4 moles of A are:
[tex]\rm 2\;mol\;A=2\;mol\;C\\\\4\;mol\;A=\dfrac{2}{2}\;\times\;4\;mol\;C\\\\ 4\;mol\;A=4\;mol\;C[/tex]
Thus, the moles of C formed by 4 moles of A are 4 moles.
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